In a displacement reaction, what happens to the metal that is displaced?

In a displacement reaction, a metal that is displaced by a more reactive metal typically undergoes a reduction process. This occurs because the more reactive metal takes the place of the less reactive metal in a compound. For instance, if metal A is more reactive than metal B, and they are involved in a reaction where A displaces B from its compound, metal B will be reduced.

Reduction, in the context of this reaction, refers to the gain of electrons by an atom or ion. When metal B is displaced, it receives electrons from the compound it's leaving, thus reducing its oxidation state. This shift in oxidation states is critical as it defines the nature of the chemical change occurring during the reaction.

By understanding the principles of oxidation and reduction, one can see how a displacement reaction leads to the reduction of the displaced metal. This is the hallmark of these types of reactions and is central to the study of redox chemistry.